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CHAPTER 4 CHEMICAL BONDING

Total questions: 50

Worksheet time: 32mins

Name
Class
Date
1.

What is the hybridization of a linear molecule?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

2.

The hybridisation of the carbon atom is?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

3.

The hybridisation of the carbon atom is?

a)

sp

b)

sp2

c)

sp3

d)

sp3d

4.

What is the hybridization of this molecule shown.

a)

sp

b)

sp2

c)

sp3

d)

sp4

5.

What is the hybridization of the Carbon atom indicated by the arrow?

a)

sp hybridization

b)

sp2 hybridization

c)

sp3 hybridization

d)

dsp3 hybridization

6.

The hybridisation of the carbon atom is?

a)

sp hybridization

b)

sp2 hybridization

c)

sp3 hybridization

d)

sp3d hybridization

7.

The hybridisation of the sulfur atom is?

a)

sp hybridization

b)

sp2 hybridization

c)

sp3 hybridization

d)

sp3d hybridization

8.

What is the hybridization of PF5?

a)

sp3

b)

sp3d

c)

sp2d2

d)

sp2

9.

Xe atom undergo

a)

sp hybridization

b)

sp2 hybridization

c)

sp3 hybridization

d)

sp3d hybridization

10.

The force of attraction between nonpolar molecules:

a)

Hydrogen Bonding

b)

Dipole - Dipole Forces

c)

Londan Dispersion Force (LDF)

d)

Ionic Forces

11.

The bond formed between atoms of the same element:

a)

nonpolar covalent

b)

polar covalent

c)

ionic bond

d)

hydrogen bond

12.

Intermolecular forces are attractions between ______.

a)

Cations and anions

b)

Atoms within a molecule

c)

Neighboring molecules

d)

Protons and electrons

13.

Which of the following might cause a hydrogen bond to form?

a)

Carbon

b)

Phosphorus

c)

Sulfur

d)

Oxygen

14.
Which of these has the strongest London forces?
a)
F2
b)
Br2
c)
Cl2
d)
I2
15.
Rank these in order of strength:
covalent bond
London forces
hydrogen bond
dipole-dipole attraction
a)
dipole-dipole>covalent bond>hydrogen bond>London
b)
London>dipole-diple>hydrogen bond>covalent bond
c)
covalent bond>hydrogen bond>dipole-dipole>London
d)
hydrogen bond>dipole-dipole>London>covalent bond
16.
What explains the very high melting and boiling point of water
a)
Strong dipole-dipole bonds between water molecules
b)
Strong hydrogen bonds between water molecules
c)
Dispersion forces which are present in all molecules
d)
Asymmetrical shape of the polar bonds.
17.

What do you call a bond that forms when electrons are transferred from one atom to another?

a)

Compound Bond

b)

Ionic Bond

c)

Crystal Bond

d)

Atom Bond

18.

This consists of two or more atoms joined together.

a)

Molecule

b)

Covalent Bond

c)

Electron-Dot Diagram

19.
Which of the following has a full valence shell?
a)
Oxygen
b)
Neon
c)
Barium
d)
Carbon
20.
How many valence electrons in this structure?
a)
6
b)
5
c)
4
d)
7
21.
An ionic bond forms when atoms ___________ electrons.
a)
gain
b)
share
c)
increase
d)
transfer
22.

What is the correct Lewis structure for BF3?

a)
b)
c)
d)

BF3 (The formula is the Lewis Structure)

23.
Predict the bond that will form between Be and F.
a)
Ionic
b)
Covalent
24.
What is a valence electron?
a)
an electron that is found in the outermost shell of an atom. 
b)
an electron found in the innermost shell of an atom.
c)
an electron found in the middle shell.
25.
What is the number of valence electrons for Beryillum?
a)
1
b)
4
c)
2
d)
7
26.
Is Hydrogen considered a metal or a non-metal?
a)
Metal
b)
Non-metal
27.
Is the following compound ionic or covalent:
AlCl3
a)
ionic 
b)
covalent
28.
What is the formula for aluminum fluoride?
a)
AlF
b)
Al2F3
c)
AlF3
d)
Al3F2
29.

Element X is in group 2, and element Y is in group 7, of the periodic table. Which ions will be present in the compound formed when X and Y react together?

a)

X+ and Y-

b)

X2+ and Y-

c)

X+ and Y2-

d)

X2- and Y+

30.

Which molecule is non-polar?

a)

H2CO

b)

SO3

c)

NF3

d)

CHCl3

31.

What happens when sodium and oxygen combine together?

a)

Each sodium atom gains one electron

b)

Each sodium atom loses one electron

c)

Each oxygen atom gains one electron

d)

Each oxygen atom loses one electron

32.

Which statement best describes the attraction present in metallic bonding?

a)

the attraction between nuclei and electrons

b)

the attraction between positive ions and electrons

c)

the attraction between positive ions and negative ions

d)

the attraction between protons and electrons

33.

When the following bond types are listed in decreasing order of strength (strongest first), what is the correct order?

a)

covalent > hydrogen > van der Waals'

b)

covalent > van der Waals' > hydrogen

c)

hydrogen > covalent > van der Waals'

d)

van der Waals' > hydrogen > covalent

34.

Which fluoride is the most ionic?

a)

NaF

b)

CsF

c)

MgF2

d)

BaF2

35.

Which substance is most similar in shape to NH3?

a)

GaI3

b)

BF3

c)

FeCl3

d)

PBr3

36.

What intermolecular forces are present in gaseous hydrogen?

a)

Hydrogen bonds

b)

Covalent bonds

c)

Dipole-dipole attractions

d)

Van der Waals' forces

37.

What are responsible for the high electrical conductivity of metals?

a)

Delocalized positive ions

b)

Delocalized valence electrons

c)

Delocalized atoms

d)

Delocalized negative ions

38.
There are more metals than non metals in the periodic table.
a)
True
b)
False
39.
At room temperature, most metals are
a)
liquid
b)
solid
c)
gas
d)
an alloy
40.

Electrons that are free to move in metals are called ..

a)

delocalized electrons

b)

oxidation number

c)

chemical bond

d)

salts

41.
What is the ability of a substance to be pulled into a thin strand?
a)
Malleability
b)
Ductility 
c)
Conductivity
d)
Solubility
42.
Why do metals have high melting points?
a)
They don't
b)
The negatively charged electrons act as a glue to hold the positively charged ions together.
c)
All the electrons become delocalised
43.

Why do metals conduct electricity and heat? Because ..

a)

They are shiny

b)

The electrons are held tightly within the lattice

c)

The electrons are delocalised and able to move

d)

The electrons are shared between two metal ions

44.

Why do metallic compounds conduct electricity as solids?

a)

core electrons are mobile, allowing electricity to flow through the metal

b)

valence electrons are mobile, allowing electricity to flow through the metal

c)

protons are mobile, allowing electricity to flow through the metal

d)

the metal cations are mobile, allowing electricity to flow through the metal

45.
In metals, the _______ electrons form a shared sea of electrons.
a)
Metallic
b)
Inner
c)
Outer
d)
Ionic
46.

The force of attraction between nonpolar molecules:

a)

Hydrogen Bonding

b)

Dipole - Dipole Forces

c)

Londan Dispersion Force (LDF)

d)

Ionic Forces

47.

Based on electronegativity values, which bond is the most polar?

a)

B-C

b)

C-O

c)

N-O

d)

O-F

48.
Covalent bonds are between...
a)
Metal and Non-metal
b)
Non-metal and Non-metal
c)
Metal and Metal
49.
What usually forms a negative ion?
a)
Non-metals
b)
metals
50.

Typically, atoms are more stable when they are

a)

bonded together

b)

apart from each other

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